Solution
a) The calibration factor is calculated by the expression below.
b) Obtain the amount of energy absorbed from 2.45 grams of ammonium nitrate
According to the equation above every mole of ammonium nitrate that dissolves absorbs 25.2Kj of energy.
SO!
Step 1) Mole of ammonium nitrate added = 2.456 /80 = 0.031 mole
Step 2) If one mole of ammonium nitrate gives off 25.2Kj of energy then.
0.031 X 25.2Kj/mol = 0.772Kj = 772joules
c) The amount of degrees drop that 2.45g of ammonium nitrate will achieve in the calorimeter is given by the expression
772 joules / 311.4
joules/C =2.48C
So the temperature of the contents of the calorimeter will be at
20.34 - 2.48 = 17.86C
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Calorimetry
exercise 4 |
A current of 1.73 A was passed through the heating coil of a calorimeter for one minute at a potential difference of 6.00 V. The temperature increased from 20.340 to 22.340 degrees Celsius. N =14, C = 12, O = 16, H =1, K =39 |
2.45grams of ammonium nitrate was dissolved in a calorimeter and the temperature dropped from 20.34C to an unknown temperature. The equation for the dissociation of ammonium nitrate is given below. NH4NO3(s) => NH4+(aq) + NO3-(aq) ΔH =+25.2 kJ/mol
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a) Calculate the calibration factor of the calorimeter. b) How much energy is absorbed by 2.45grams of ammonium nitrate? c) What is the final temperature of the contents of the calorimeter? |
Solution |